Determine the heat evolved in kj when 150 g of aluminum...

Determine the heat evolved (in kJ) when 15.0 g of Aluminum reacts with excess iron (III) oxide. Is this reaction endothermic or exothermic? Show your work. 2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) ΔH°rxn = -849 kJ/mol

Transcript

00:01 Hello, students.

00:02 So in this question, you have been given this reaction.

00:04 So in the reaction, what is happening? we have aluminium.

00:06 It is reacting with fp2 -03 in excess and it forms the aluminum oxide and f -p as solid.

00:14 And the heat released or the heat of permission of this reaction is minus 8 for 9 kilojoules per mode.

00:21 And you have to find out the delta h -0 for if we are given with aluminium 515 grams.

00:28 So before that, we have to find out the delta h -0 .4.

00:30 If we are given with aluminium 515 grams.

00:30 Find we have to deal with the moles so molar mass if we see molar mass of aluminum of aluminum is 26 .982 gram per mole right these are the values of the molar mass so now if we say that here how many moles in this reaction if two moles if two moles of aluminum gives out delta h delta h is equal to delta h not is equal to minus 8 for 9 kilojoules per molar per mole per mole right so we can say for one mole it has the mass of so this is this is the molar mass so we can also say that one mole it is equals to one more that is only the meaning of molar mass right so for one mole we have one mole of an aluminum the mass will be is equal to 26 .982 grams okay so if we have two moles two moles means two multiply by 26 .9 98 grams of aluminum it gives out delta h s delta h as minus 849 kilojoules per more fine so now proceeding again we are given with the mass of 15 grams so if we have to find out for the 1 gram unit room method we are going to apply over here delta h not is equals to minus 8 4 9 divided by 2 multiply by 2 26 .9 8 .9 grams right here we have kilojoules per mole also so in questions we have asked for the 15 grams of aluminium it is delta h is equal to minus 849 divide by 2 multiply by 26 .98 multiply by 15.

02:48 All right...

Question

Determine the heat evolved (in kJ) when 15.0 g of Aluminum reacts with excess iron (III) oxide. Is this reaction endothermic or exothermic? Show your work. 2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) ΔH°rxn = -849 kJ/mol

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